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Given the following reaction: 2 NO(g) + O2(g) <--> 2 NO2(g), what is the equilibrium constant (K), if the concentrations at equilibrium are [NO] = 0.0542 M, [O2] = 0.127 M, and [NO2] = 15.5 M?
Group of answer choices

A. K = 2.35 x 102

B. K = 2.54 x 10-1

C. K = 6.44 x 105

D. K = 3.4 x 103

Sagot :

Mickymike92idn

The equilibrium constant of a reaction, [tex]K_{c}[/tex]  = 6.44 * 10⁵; option C.

What is equilibrium constant of a reaction?

Equilibrium constant, [tex]K_{c}[/tex] of a reaction is a measure of the ratio of the equilibrium concentration of the products of a reaction, to the equilibrium concentration of the reactants; with each concentration raised to the exponent corresponding to the coefficient in the balanced equation of the reaction.

[tex]K_{c} = \frac{(products)^{a}}{(reactants)^{b}}[/tex]

The balanced equation of the given reaction is as follows:

  • 2 NO (g) + O₂ (g) ⇄ 2 NO₂ (g)

The concentrations at equilibrium of the species are as follows:

[NO] = 0.0542 M,

[O₂] = 0.127 M, and

[NO₂] = 15.5 M

Equilibrium constant, [tex]K_{c}[/tex] = (15.5)²/(0.127) * (0.0542)²

[tex]K_{c}[/tex]  = 6.44 * 10⁵

In conclusion, the equilibrium constant of a reaction, tells on in which direction, the reaction is favored at equilibrium.

Learn more about equilibrium constant at: https://brainly.com/question/12270624

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